WO2012134954A1 - Procédés et appareil pour réguler des vitesses de réaction de réactions chimiques par l'application d'un champ magnétique - Google Patents

Procédés et appareil pour réguler des vitesses de réaction de réactions chimiques par l'application d'un champ magnétique Download PDF

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WO2012134954A1
WO2012134954A1 PCT/US2012/030141 US2012030141W WO2012134954A1 WO 2012134954 A1 WO2012134954 A1 WO 2012134954A1 US 2012030141 W US2012030141 W US 2012030141W WO 2012134954 A1 WO2012134954 A1 WO 2012134954A1
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WIPO (PCT)
Prior art keywords
magnetic field
reaction
chemical
reactants
graphite
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PCT/US2012/030141
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English (en)
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Reginald B. LITTLE
James W. Mitchell
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Howard University
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Priority to CA2830899A priority Critical patent/CA2830899C/fr
Priority to US14/006,080 priority patent/US9511343B2/en
Priority to GB1318430.4A priority patent/GB2504025B/en
Priority to DE112012001442T priority patent/DE112012001442T5/de
Publication of WO2012134954A1 publication Critical patent/WO2012134954A1/fr

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    • B—PERFORMING OPERATIONS; TRANSPORTING
    • B01—PHYSICAL OR CHEMICAL PROCESSES OR APPARATUS IN GENERAL
    • B01J—CHEMICAL OR PHYSICAL PROCESSES, e.g. CATALYSIS OR COLLOID CHEMISTRY; THEIR RELEVANT APPARATUS
    • B01J8/00—Chemical or physical processes in general, conducted in the presence of fluids and solid particles; Apparatus for such processes
    • B01J8/02—Chemical or physical processes in general, conducted in the presence of fluids and solid particles; Apparatus for such processes with stationary particles, e.g. in fixed beds
    • B—PERFORMING OPERATIONS; TRANSPORTING
    • B01—PHYSICAL OR CHEMICAL PROCESSES OR APPARATUS IN GENERAL
    • B01J—CHEMICAL OR PHYSICAL PROCESSES, e.g. CATALYSIS OR COLLOID CHEMISTRY; THEIR RELEVANT APPARATUS
    • B01J19/00—Chemical, physical or physico-chemical processes in general; Their relevant apparatus
    • B01J19/08—Processes employing the direct application of electric or wave energy, or particle radiation; Apparatus therefor
    • B01J19/087—Processes employing the direct application of electric or wave energy, or particle radiation; Apparatus therefor employing electric or magnetic energy
    • B—PERFORMING OPERATIONS; TRANSPORTING
    • B82—NANOTECHNOLOGY
    • B82Y—SPECIFIC USES OR APPLICATIONS OF NANOSTRUCTURES; MEASUREMENT OR ANALYSIS OF NANOSTRUCTURES; MANUFACTURE OR TREATMENT OF NANOSTRUCTURES
    • B82Y30/00—Nanotechnology for materials or surface science, e.g. nanocomposites
    • B—PERFORMING OPERATIONS; TRANSPORTING
    • B82—NANOTECHNOLOGY
    • B82Y—SPECIFIC USES OR APPLICATIONS OF NANOSTRUCTURES; MEASUREMENT OR ANALYSIS OF NANOSTRUCTURES; MANUFACTURE OR TREATMENT OF NANOSTRUCTURES
    • B82Y40/00—Manufacture or treatment of nanostructures
    • C—CHEMISTRY; METALLURGY
    • C01—INORGANIC CHEMISTRY
    • C01B—NON-METALLIC ELEMENTS; COMPOUNDS THEREOF; METALLOIDS OR COMPOUNDS THEREOF NOT COVERED BY SUBCLASS C01C
    • C01B32/00—Carbon; Compounds thereof
    • C01B32/15—Nano-sized carbon materials
    • C01B32/182—Graphene
    • C01B32/194—After-treatment
    • C—CHEMISTRY; METALLURGY
    • C01—INORGANIC CHEMISTRY
    • C01B—NON-METALLIC ELEMENTS; COMPOUNDS THEREOF; METALLOIDS OR COMPOUNDS THEREOF NOT COVERED BY SUBCLASS C01C
    • C01B32/00—Carbon; Compounds thereof
    • C01B32/20—Graphite
    • C01B32/21—After-treatment
    • C01B32/23—Oxidation
    • B—PERFORMING OPERATIONS; TRANSPORTING
    • B01—PHYSICAL OR CHEMICAL PROCESSES OR APPARATUS IN GENERAL
    • B01J—CHEMICAL OR PHYSICAL PROCESSES, e.g. CATALYSIS OR COLLOID CHEMISTRY; THEIR RELEVANT APPARATUS
    • B01J2219/00—Chemical, physical or physico-chemical processes in general; Their relevant apparatus
    • B01J2219/08—Processes employing the direct application of electric or wave energy, or particle radiation; Apparatus therefor
    • B01J2219/0873—Materials to be treated
    • B01J2219/0881—Two or more materials
    • B01J2219/089—Liquid-solid
    • B—PERFORMING OPERATIONS; TRANSPORTING
    • B01—PHYSICAL OR CHEMICAL PROCESSES OR APPARATUS IN GENERAL
    • B01J—CHEMICAL OR PHYSICAL PROCESSES, e.g. CATALYSIS OR COLLOID CHEMISTRY; THEIR RELEVANT APPARATUS
    • B01J2219/00—Chemical, physical or physico-chemical processes in general; Their relevant apparatus
    • B01J2219/08—Processes employing the direct application of electric or wave energy, or particle radiation; Apparatus therefor
    • B01J2219/0873—Materials to be treated
    • B01J2219/0892—Materials to be treated involving catalytically active material

Definitions

  • a method of promoting and selecting a chemical reaction having the steps of: admixing chemical precursors, wherein at least one chemical precursor or its intermediate is magnetic (e.g., a para-magnetic orferro-magnetic magnetic precursor); and applying a supplemental magnetic field to the chemical precursors, wherein the chemical reaction is promoted.
  • the initial reaction temperature can be in the range of about 25° to 1000° Celsius, though in one approach a range of about 25° to about 75° Celsius is provided.
  • the at least one chemical precursor can be selected from the group of graphite, graphene, coal, diamond, cellulose, proteins, various combinations thereof, and the like.
  • the at least one chemical precursor or its intermediate can contain carbon, wherein during the step of applying the supplemental magnetic field, the carbon undergoes a dynamic transition to become magnetic.
  • the carbon undergoes a dynamic transition to become ferromagnetic.
  • the supplemental magnetic field is in the range of up to about 50 Tesla (T). in other embodiments, the supplemental magnetic field is about 0.5 T.
  • the supplemental magnetic field can constant during the reaction.
  • the applied magnetic field can vary over time in the range of about 0 to 500 seconds and also vary in space in the range of about 0 to 1 micron.
  • the promoted chemical reaction can occur in an oxygenated environment in the range of about 1 to 80 percent. In another embodiment, the promoted chemical reaction can occur in a pressure range of about 10 --9 to 10 8 atm. [0010] In one approach, the method can also include the step of admixing an additional magnetic alloy catalyst.
  • the additional magnetic alloy catalyst can be selected from the group of iron, cobalt, neodymium, nickel, combinations thereof, and the like. In one approach the additional magnetic alloy catalyst can be in the range of about 1 to 40 percent weight of the total reactants.
  • the chemical reaction can be configured for the oxidation of graphite to graphene oxide, in another approach, the chemical reaction can be configured for the nitration of graphene. In yet another approach, the chemical reaction can be configured for the combustion of coal. In still another approach, the chemical reaction can be configured to functionalize graphene for prope!lants.
  • the chemical reaction can further add the step of adding reagents selected from the group of perchlorates, borates, chromates, oxides, cobaltates, nickelates, vandates, various combinations thereof, and the like.
  • the promoted chemical reaction can occur in an anaerobic environment, !n one approach this can include anaerobic environment that includes Argon gas.
  • Another approach provides a composition formed by a method of promoting a chemical reaction having the steps of admixing chemical precursors, wherein at least one chemical precursor or its intermediate contains carbon; and applying a magnetic field to the chemical precursors, wherein the chemical reaction is promoted.
  • a method of controlling a reaction rate of a chemical reaction having the steps of mixing chemical reactants to provide a reaction mixture, at least one chemical reactant being magnetic; and applying a magnetic field to the reaction mixture, the magnetic field being applied to effect a control of the rate of a chemical reaction between the reactants in the reaction mixture, the magnetic field being effective to change the reaction rate over a chemical reaction between the same reactants at the same pressure and temperature where the reaction mixture is not exposed to the magnetic field.
  • the reaction mixture can have an initial reaction temperature in the range of about 25° to 1000° Celsius, or in some embodiments an initial reaction temperature in a range of about 25° to about 75° Celsius, tn this approach, at least one chemical reactant can be selected from the group of graphite, graphene, coal, diamond, cellulose, proteins, combinations thereof, and the like. In other embodiments, one of the reactants can be sulfuric acid, NaNO 3 , KMnO 4 and mixtures thereof.
  • the magnetic field can in the range of from about 0.5 to about 50 Tesla and in other embodiments, the magnetic field can be in the range of from about 0.5 to about 50 Tesla. In some embodiments the reaction rate can be increased or decreased with the reaction being exposed to the magnetic field.
  • an apparatus configured to effect a chemical reaction during which the reaction is exposed to a magnetic field, the apparatus having a chamber configured to blend chemical reactants and react the chemical reactants, at least one first chemical reactant selected from the group consisting of graphite, graphene, coal, diamond, cellulose, proteins, and combinations thereof and at least one second reactant selected from the group consisting of sulfuric acid, NaNO 3 , KMnO 4 and mixtures thereof; and a magnetic field source device effective to expose the first and second reactants to a magnetic field magnetic field within the chamber, the magnetic field source device effective for providing a magnetic field in the range of from about 0.5 to about 50 Tesla.
  • the chamber can be effective for containing reactions which have a temperature in the range of about 25° to 1000° Celsius.
  • method of increasing a reaction rate of a chemical reaction having the steps of mixing chemical reactants to provide a reaction mixture, at least one chemical reactant being magnetic; and applying a magnetic field to the reaction mixture, the magnetic field being applied to effect an increase of the rate of a chemical reaction between the reactants in the reaction mixture, the magnetic field being effective to change the reaction rate by at least 14 percent over a chemical reaction between the same reactants at the same pressure and temperature after the same time period of reaction where the reaction mixture is not exposed to the magnetic field.
  • FIGURE 1 comprises a Mass Spectra during Reaction of Graphite + H 2 SO 4 + NaNO 3
  • FIGURE 2 comprises a Mass Spectra during Reaction of Graphite + H 2 SO 4 + NaNO 3
  • FIGURE 3 comprises a Mass Spectra during Reaction of Graphite + H 2 SO 4 + NaNO 3
  • FIGURE 4 comprises a Mass Spectra during Reaction of Graphite + H 2 SO 4 + NaNO 3
  • FIGURE 5 comprises a Mass Spectra during Reaction of Graphite + H 2 SO 4 + NaNO 3
  • FIGURE 6 comprises a Mass Spectra during Reaction of Graphite + H 2 SO 4 + NaNO 3
  • FIGURE 7 comprises a Mass Spectra during Reaction of Graphite + H 2 SO 4 + NaNO 3
  • Oxidation-reduction reactions in particular combustion chemistry play an important role in the biosphere and geosphere. A greater understanding and control of such chemistry is desirable and beneficial to centuries.
  • methods of magnetic and thermal activation are disclosed to modulate oxidation reduction reactions so as to improve conversion, efficiency of energy transformations and rates of such reactions.
  • a new chemistry of relativistic electron transfer is introduced. The new magnetic induction and control of oxidation reduction are demonstrated for the Hummer Method of graphite oxidation by potassium permanganate, sodium nitrate and sulfuric acid.
  • the embodiments described herein provide systems and methods of the application of magnetism as it relates to chemical oxidation-reduction of carbonaceous substances and the accelerative, the power output, and the selective chemistry of such carbonaceous reactions.
  • the embodiments provide improvements in rates of oxidative-reductive reactions and the operating temperatures for higher energy conversions of such chemical energies to work.
  • the effect of the present embodiments can be shown in reactions using solid and liquid phase reactants. Accordingly, the methods and compositions can improve the efficiency of chemical energy conversions by modulating operating temperatures and rates of oxidative-reductive reactions.
  • ferromagnetism in carbon can be by way of example harnessed to accelerate, decelerate and control energetic and product distribution of such chemical reactions.
  • the internal, inherent magnetic properties of other reactants and oxidants that contain second series and 3d elements of the periodic table can also be harnessed to control the oxidative reductive chemistry.
  • Illustrative reactions of this type are described herein to demonstrate the presented methods and system embodiments.
  • the use of magnetization with optional thermal activation for organizing, synchronizing, selecting, decelerating, accelerating and orchestrating chemical reactions can provide several energy saving
  • the present embodiments can be demonstrated and realized using the recent discovery of graphene (one-atom-thick planar sheets of sp 2 -bonded carbon atoms densely packed in a honeycomb crystal lattice) and the unique Dirac electronic symmetry of graphene* graphite.
  • These embodiments can allow new uses of magnetization for control of chemical kinetics, dynamics and catalysis for chemically altering Dirac electronic symmetry and for thereby implementing a new relativistic chemistry.
  • induced magnetism can be used to exploit the Dirac symmetry for new chemical kinetics. As reactions occur, the magnetic field can organize and compress the reactants, intermediates and products in space-time.
  • Reactions can occur in magnetic and nonmagnetic environments, but the external magnetic field can slow the reaction rate so that as temperature rises more conversions simultaneously can occur at times with more powerful and accelerated release of energy. Accordingly, the externally induced magnetic field may control such energy releases to raise furnace temperature for better efficient energy conversion to work.
  • engines and generators can operate by oxidation of carbon, hydrocarbons and other carbonaceous substances by thermal conditions for activating the reactions.
  • carbon sources are provided with activation energy for breaking bonds of the reactants for subsequent new bond formations and for forming the products: e.g., CO 2 and H 2 0.
  • the exothermicity of oxidative reductive reactions provides subsequent energy to sustain activation of the combustion.
  • the higher temperatures can also push reactants apart to expand the reacting media and the subsequent exothermicity further pushes reactants and intermediates apart to diminish combustion yield and instantaneous power.
  • an induced external magnetic field is provided to oppose the subsonic thermal expansion of reactants and intermediates during combustion reactions.
  • the external magnetic field can orient reactants more rapidly relative to the stoichastic orientation in zero applied magnetic field.
  • the external magnetic field can induce organized and synchronized rotations of the reactants relative to the stoichastic, random and chaotic motions in zero applied magnetic field.
  • the magnetic field can better hold paramagnetic reactants and paramagnetic intermediates together at a given temperature relative to the stoichastic dispersion of the reactants and intermediates in zero applied magnetic field.
  • the external magnetic field can compress reactants and intermediates for more organized, synchronized oxidative reductive reactions relative to oxidation-reduction reaction with no applied magnetic field.
  • Potential applications for the present embodiments can include, for example: device fabrication of graphene based nano-electronics in magnetic field; acceleration of oxidation of carbonaceous materials, such as coal, for higher efficiency of coal burning power plants in magnetic field; shifting in equilibrium operating conditions of water gas shift reaction on graphene or graphite in magnetic field - Example:
  • methods and systems are provided for magnetic acceleration, deceleration, control and shift in chemical reaction kinetics and dynamics of graphite graphene and H 2 SO 4 in strong oxidants (e.g., KMnO 4 ,NaNO 3 , any powdered or solid carbonaceous materials in a direct reaction with O 2 ) involving that of faster oxidative reductive kinetics to accelerated reaction and shift in dynamics for nitration and sulfonation of graphene.
  • strong oxidants e.g., KMnO 4 ,NaNO 3 , any powdered or solid carbonaceous materials in a direct reaction with O 2
  • Magnetic field organization of the intermediates can form aromatic polyoxoanionic complexes (Mn x O y -z -N a O b -c , Mn x O y -z -S a O b -c and Mn x O y -z - Mn a O b -c ) of these oxidative species for their magnetically driven orientations for accelerated aromatic multi- electron transfer (Dirac Chemistry) reactions with graphite-graphene reductants.
  • aromatic polyoxoanionic complexes Mn x O y -z -N a O b -c , Mn x O y -z -S a O b -c and Mn x O y -z - Mn a O b -c
  • the magnetizations and protonations of these oxidative, anionic complexes can contribute more thermodynamics stability and kinetic lability to these polyoxoanionic complexes (Mn x O y -z -N a O b -c , Mn x O y -z -S a O b -c and Mn x O y -z - Mn a O b -c ).
  • the present embodiments can provide magnetic field induced aromatic symmetry into such polyoxoanions of Mn x O y -z -N a O b -c , Mn x O y -z -S a O b -c and Mn x O y -z - Mn a O b -c for similar Dirac electron symmetry as in pi ( ⁇ ) aromatic electrons in graphene with the consequent synchronization of multiple, fused, oxidizing, aromatic-like oxidative polyoxoanionic-complexes for reducing, aromatic graphene thereby for faster Dirac aromatic graphene oxidative reductive chemistry.
  • the external magnetic field also enhances the organization of protons of the strong acid for their concerted protonations of the Mn x O y -z -N a O b -c , Mn x O y -z -S a O b -c and Mn x O y -z - Mn a O b -c polyoxoanionic complexes for the concerted breakages of N-O and Mn-O bonds.
  • the concerted breakages of N-O and Mn-O bonds occur relativistically.
  • the magnetic field then orient
  • compositions can include materials of preferred carbonaceous states that are highly crystalline graphite.
  • Coal and amorphous carbons can also be applied and can also be oxidized and nitrated by the present methods.
  • Other reagents such as perchlorates, borates, chromates, oxides, cobaltates, nickelates, vandates, and the like, are also applicable to provide further enhanced efficiency of chemical reaction.
  • [0037] [Exemplary tests for compositions using systems, methods and devices for magnetic acceleration and shift in chemical reaction kinetics and dynamics can be generally described as graphite + oxygen +/- an induced magnetic field as a catalyst to provide and exothermic reaction (e.g., a flame or a flash). Specific tests were as follows:
  • the initial CO 2 levels in Figure 1 for magnetic oxidation are greater than the initial CO 2 levels in Figure 1 for non-applied external magnetic oxidation.
  • the CO 2 is therefore formed with smaller induction time and more rapidly by applying external magnetic field to the oxidation under aerobic atmosphere.
  • the faster CO 2 production in the applied external magnetic field for the aerobic oxidation may result due to the applied magnetic field orienting p* (aq) and O 2 (g) for multiple spin exchange with reactants to allow multiple electron transfers. Due to the limited amount of initial reactants for the aerobic oxidation without applied external magnetic field (in Figure 1), there was a faster rise in CO 2 amount before the peak at 8 minutes and a faster fall in CO 2 level after the peak relative to the kinetics for the aerobic oxidation without applied external magnetic field (in Figure 1).
  • the second derivative kinetics are also presented and compared for the graphitic aerobic oxidations with and without applied magnetic field.
  • the second derivative kinetics revealed differences for the oxidation rates with and without applied magnetic field.
  • the second derivative kinetics express the rates of change in rates of the reactions. It is observed that the applied magnetic field causes a hysteresis in the kinetics of aerobic oxidation. Such hysteresis suggests the possibility of reversible oxidative-reductive chemistry of graphite oxidation under suitable thermal and magnetic conditions.
  • the reaction rate exhibited hysteresis of slowly increasing, then rapidly decreasing, then slightly increasing for the oxidation under applied magnetic field.
  • the inert Ar background gas diminished flashes and flaming during graphite oxidation.
  • the Ar is less buoyant than air, affecting oxidation by suppressing the flashes during the oxidation.
  • the Ar unlike the air exposed system is forced through the system by the pressure of the Ar tank.
  • the anaerobic oxidation in magnetic field in Ar background was observed to occur at a faster rate than the anaerobic oxidation in Ar without applied external magnetic field.
  • the maximum reaction rate in Ar under applied magnetic field was
  • This difference in hysteretic behavior between aerobic (in O 2 ) and anaerobic (in Ar) graphite oxidations with no applied magnetic field may be understood as the aerobic conditions removes spin order from reactants by spin exchange of the reactants (graphite + Mn x O y -z -N a O b -c , Mn x O y - z - S a O b -c and Mn x O y -z - Mn a O b -c ) with the incoming paramagnetic O 2 in air for the aerobic system.
  • O 2 molecular spins exchange with p + (aq) and or the polyoxoanionic complexes and graphite intermediates of the strongly acidic media.
  • O 2 (g) couples more strongly than p + (aq) to external magnetic field. Therefore the dynamics on aerobic O 2 (g) atmosphere are more sensitive to external magnetic field than dynamics in anaerobic atmosphere.
  • the O 2 (g) in gas phase can couple better to the weak magnetic field than the p*(aq) in the water.
  • the spin polarization and internal magnetism cause the cooperative hysteresis. So by removing spin polarization of reactants by incoming O 2l the hysteresis of the reaction is diminished.
  • Figure 3 compares the oxidation in air with the oxidation in Ar without an externally applied magnetic field at 25° C.
  • the oxidation kinetics in Air are much faster than the oxidation kinetics in Ar without external magnetization.
  • the faster oxidation kinetics in Air may be due to the paramagnetic nature of O 2 (g) and it may be due to the increased direct oxidation of the graphite by gaseous atmospheric O 2 (g) as the mixture heats from its exothermicity.
  • the paramagnetic O 2 (g) molecule affects the internal magnetism in the reaction of graphite with H 2 SO 4 , KMnO 4 and NaNO 3 as the O 2 exchanges spin momentum with the intermediates as the oxidation proceeds.
  • Such exchange of spin momentum allows the increased acid oxidation as it allows continued electron transfer between the increasingly magnetic graphitic reductants and magnetic oxidants (Mn x O y -z -N a O b -c , Mn x O y -z -S a O b -c and Mn x O y -z - Mn a O b -c ) by removing spin polarization and alleviating frustrated e- transfer by Pauli Exclusion Principle so that the multi- electron transfers become allowed and occur by O 2 (g) buffering the necessary spin momentum thereby allowing multi-electron transfer to occur.
  • O 2 (g) is paramagnetic and quite remarkably, it was observed that the external magnetic field and developing internal ferromagnetism opposed Henry's Law and the thermal effect of lowering O 2 (g) solubility at higher temperatures by magnetically increasing the paramagnetic O 2 (g) solubility and concentration in aqueous media in spite of the higher temperature at 75° C for faster oxidation and greater CO 2 production at 75° C relative to 25° C and organization of the graphite oxidation in the water solution.
  • the greater effect of magnetism relative to Henry's Law follows from the development of stronger ferromagnetism in graphite oxide and defective graphite relative to the initial graphite. Such greater ferromagnetism of the graphite
  • intermediates and graphene oxide present much stronger magnetic attraction to paramagnetic oxygen molecules and Mn x O y -z -N a O b -c , Mn x O y -z -S a O b -c and Mn x O y -z - Mn a O b -c relative to the weaker van der Waals and London forces classically that cause the Henry's Law.
  • the ferromagnetism of graphite oxide pulls paramagnetic O 2 (g) to the ferromagnetic graphite oxide. In this way, the Henry's Law is opposed so faster oxidation occurs from O 2 (g) in spite of higher temperatures and Henry's Law.
  • the diamagnetic CO 2 is also pushed away from the oxidative reductive reactions under magnetization to further drive the equilibrium toward the right, producing more CO 2 and burning more graphite.
  • the effect of less Henry's Law to magnetically uptake of CO 2 (g) is revealed in the slower decrease in reaction rate after peak in the Air, relative to the faster decrease in reaction rate in Ar for a hysteretic cooperative effect observed in the aerobic oxidation under magnetic field.

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Abstract

La présente invention a pour objet des procédés et un appareil pour réguler des vitesses de réaction de réactions chimiques. Les procédés peuvent comprendre les étapes consistant à mélanger des réactifs chimiques pour fournir un mélange réactionnel, au moins un réactif chimique étant magnétique ; et à appliquer un champ magnétique au mélange réactionnel, le champ magnétique étant appliqué pour effectuer une régulation de la vitesse d'une réaction chimique entre les réactifs dans le mélange réactionnel, le champ magnétique étant efficace pour modifier la vitesse de réaction par rapport à une réaction chimique entre les mêmes réactifs aux mêmes pression et température lorsque le mélange réactionnel n'est pas exposé au champ magnétique.
PCT/US2012/030141 2011-03-25 2012-03-22 Procédés et appareil pour réguler des vitesses de réaction de réactions chimiques par l'application d'un champ magnétique WO2012134954A1 (fr)

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CA2830899A CA2830899C (fr) 2011-03-25 2012-03-22 Procedes et appareil pour reguler des vitesses de reaction de reactions chimiques par l'application d'un champ magnetique
US14/006,080 US9511343B2 (en) 2011-03-25 2012-03-22 Methods and apparatus to control reaction rates of chemical reactions by applying a magnetic field
GB1318430.4A GB2504025B (en) 2011-03-25 2012-03-22 Methods to control reaction rates of chemical reactions by applying a magnetic field
DE112012001442T DE112012001442T5 (de) 2011-03-25 2012-03-22 Verfahren und vorrichtungen zum steuern von reaktionsraten von chemischen reaktionen durch anlegen eines magnetfeldes

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US201161467708P 2011-03-25 2011-03-25
US61/467,708 2011-03-25

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US20140147369A1 (en) 2014-05-29
CA2830899C (fr) 2020-03-31
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DE112012001442T5 (de) 2013-12-19

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